Sample Written Report

Topics: Periodic table, Chemical element, Atomic number Pages: 5 (1105 words) Published: January 23, 2013
Claro M. Recto Information and Communication Technology High School

Doña Aurora St., Claro M. Recto, Angeles City

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1. Trace the development of the Modern Periodic Table of Elements;

2. Describe the contributions of early scientists in the development of the Periodic Table of Elements; and

3. Analyze the basis of arrangement of elements in the Modern Periodic Table.


The periodic table is a table in which all of the known elements are listed. The table arranges the elements in order of increasing proton number to show the similarities of chemical elements. Therefore elements with structural similarities & atomic number are placed together. These elements can be placed into two different categories, metals & non-metals.

The early years of the 19th century witnessed a rapid development in chemistry. The art of distinguishing similarities and differences among atoms prompted scientists to devise a way of arranging the elements. Relationships were discerned more readily among the compounds than among the elements; thus, the classification of elements lagged many years behind the classification of compounds.

Development of the Periodic Table

It was in 1817 when Johann Wolfgang Döbereiner showed that the atomic weight of strontium lies midway between those of calcium and barium. Some years later he showed that other such “triads” exist (chlorine, bromine, and iodine and lithium, sodium, and potassium).

Another way of classifying the elements was later proposed by John Alexander Reina Newlands in 1864. He proposed that elements be classified in the order of increasing atomic weights.

As a result of an extensive correlation of the properties and the atomic weights of the elements in 1869, Dmitri Inovich Mendeleev proposed the periodic law, which states that “the elements arranged according to the magnitude of atomic masses show a periodic change of properties.”

Mendeleev’s Version of Periodic Table

The rows 1 to 7 are called periods. The columns I A on the left to 0 on the right are known as groups. Elements with similar properties fall into vertical columns (groups) and horizontal rows (periods), which form the table. The columns in the table are called Groups. The elements in a group have the same number of electrons in their outer shell.

Arrangement of the Elements According To Groups

Group I A - The Alkali Metals

Group 1 elements are soft silvery metals. They react strongly with water. The further down the group you go, the more violent this reaction is. These alkali metals are usually stored under oil to protect them from moisture and oxygen. They all have one electron in their outer shells.

Group II A – The Alkaline Earth Metals
This group consists of all metals that occur naturally in compound form. They are obtained from mineral ores and form alkaline solutions. These are less reactive than alkali metals. Group III A – The Aluminum Group

The elements in this group are fairly reactive. The group is composed of four metals and one metalloid which is boron. Group IV A – The Carbon Group
This group is composed of elements having varied properties because their metallic property increases from top to bottom meaning the top line, which is carbon, is a nonmetal while silicon and germanium are metalloids, and tin and lead are metals. Group V A – The Nitrogen Group

Like the elements in group IV A, this group also consists of metals, nonmetal and metalloids. Group VI A – The Oxygen Group
This group is called the oxygen group since oxygen is the top line element. It is composed of three nonmetals, namely, oxygen, sulfur and selenium, one metalloid, (tellurium) and one metal (polonium) Group VII A – The Halogens

This group is composed of entirely nonmetals. The term...
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